LA City College
Dr. Han
Chem 60 Study Guide (EXAM #4)
In order to do well on this exam, the student MUST master the following material:
Chapter 12:
Know the differences between a cation and an anion (by electronic configuration, charge, etc.)
What is isoelectronic? Know its meaning and understanding it by its electronic configuration and/or
charge of the ion or atom.
Know how to draw a Lewis dot diagram form an ionic compound by its ion charge and/or valence
electrons.
Know the differences between an ionic bond and a covalent bond.
Know the differences between a pure covalent bond and a polar covalent bond.
Understand electronegativity and apply it to determination of the bond type a pair of atoms.
Know how to draw Lewis dot diagrams for molecules which disobey the octet rule (radicals, expanded).
Know what metallic bonds are and understand delocalization and location with respect to flow of
electrons.
Chapter 13:
Know what a Lewis dot diagram for molecules (see procedure in section 13.1).
Understand how electron-pair repulsion affects the geometry of a covalent molecule.
Determine the electronic geometry, molecular geometry, bond angle, polarity, and drawing of any
covalent molecule or ion.
Understand what “octet” is relative to a Lewis dot diagram.
Illustrate a dipole moment for a molecule in justifying the polarity of a molecule.
Briefly know what isomers are in relatively to an organic molecule.
Know the various functional groups in typical organic molecules.
Chapter 14:
Know the properties of gases (revisit chapter 4) including the kinetic molecular theory.
Know Boyle’s and Charles’s Law (revisit chapter 4).
Know Avogadro’s Law.
Know the intangibles of Ideal Gas Law and perform calculations (n, V, T, P) along with density and
molar mass.
Know molar volume at STP and perform stoichiometric calculations.
Understand gas stoichiometry in performing a problem (both molar volume and ideal gas law).
Understand volume-volume gas stoichiometry.
Chapter 15:
Understand Dalton’s Partial Pressures.
Know the properties of liquids.
Know the five total intermolecular forces (dispersion/induced dipole, dipole-dipole, hydrogen bonding,
metallic bonding, and ionic bonding) by studying various physical properties (melting point, boiling
point, rate of evaporation, viscosity, vapor pressure, and surface tension)
Know the effect temperature has with respect to collisions in its effective evaporation rate and its relative
kinetic energy.
Know the six physical processes (melting, boiling, sublimation, deposition, vaporization, condensation).
Know water and its importance in its molecule.
Know the various types of solids (ionic, molecular, network, and metallic) and examples of each type.
Know also differences in these solids (ionic, molecular, network, and metallic).
Perform energy calculations (for heat) with aid of specific heat constants of a substance.
Calculate the amount of energy needed for a process involving water (ice, liquid, and/or steam).
LA City College
Dr. Han
NOTE: Students MUST know all of the prefix conversions (i.e. 1000g = 1kg, 10 mm = 1 cm, etc.)
and I will assist US-metric and US equalities as needed, Review labs relevant to chapters 12-15.
Also, look at the assigned problems at OWL and in your textbook. Make sure you understand
the concepts relative to the question in each section. Good luck!!!
PRACTICE Problems
This is just to see how you would handle the short answer, fill-in, and problem solving portion
of the exam. Expect no key to be provided. If you’re struggling with any of these questions,
please refer back to your textbook and reread the section which best explain the concept(s) of
the question.
1. Fill in the table below.
a. Draw the Lewis dot structure of the molecule. Use lines for shared electrons and
dots for electrons (non-bonded). If you have an ion, please bracket the structure
with its corresponding charge.
b. Determine the molecular geometry of the molecule/ion.
c. Determine the electronic geometry of the molecule/ion.
d. Determine if the molecule is overall polar or nonpolar.
e. Determine the bond angle of the molecule or ion.
Molecule
Lewis Dot
Molecular
Electronic
Polarity
Bond Angle
Diagram
Geometry
Geometry
NO21-
X
CO
H2S
HCN
CCl4
2. What volume of hydrogen (in mL) is produced at STP when 45.1g of magnesium reacts
with excess 6.0M HCl?
LA City College
3.
Dr. Han
Rank the following substances from lowest to highest vapor pressure.
CH4, NH3, Ag, NaCl, CH3OCH3
4. Why does water have a higher boiling point than hydrogen sulfide (H2S)?
5. A 4.37 gram sample of a certain diatomic gas occupies a volume of 3.00-L at 1.00 atm and
a temperature of 45oC. Identify this gas. HINT: The identity of this gas has a formula of
X2 where X is the element.
6. Determine which of the following elements in each bond will have the partial positive
charge (+) & partial negative charge (-). Use your electronegative table in your
textbook.
a. C-F
d. P-Br
7.
b. N-Cl
e. S-I
c. B-O
f. As-Cl
What volume of CO2 will be produced at STP if 6.5L of O2 mixes with excess C3H8 (g)?
REACTION (unbalanced): __ C3H8 (g) + __ O2 (g)  __CO2 (g) + __H2O (g)
8. A sample of 35.1g of methane gas (CH4) has a volume of 5.20L at a pressure of 2.70 atm.
Calculate the temperature in Kelvins and Celsius.
9. Name three ions (cations and/or ions) which are isoelectronic to Ne. Please provide the
complete electronic configuration of Ne.
10. How much energy in J will be needed to convert 125 grams of steam at 125 oC ice at -20.
oC? Is this exothermic or endothermic? Show a phase diagram.